1. Chapter 4 Chemical Bonding: The Ionic Bond Model

2. Chapter 4 Table of Contents Copyright © Cengage Learning. All rights reserved 2 4.1Chemical Bonds 4.2Valence Electrons and Lewis Symbols 4.3The Octet Rule 4.4The Ionic Bond Model 4.5The Sign and Magnitude of Ionic Charge 4.6Lewis Structures for Ionic Compounds 4.7Chemical Formulas for Ionic Compounds 4.8The Structure of Ionic Compounds 4.9Recognizing and Naming Binary Ionic Compounds 4.10Polyatomic Ions 4.11Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions

3. Chemical Bonds Section 4.1 Copyright © Cengage Learning. All rights reserved 3 A Chemical Bond Attractive force that holds two atoms together in a more complex unit. Form as a result of interactions between electrons found in the combining atoms.

4. Chemical Bonds Section 4.1 Copyright © Cengage Learning. All rights reserved 4 Two Types of Chemical Bonds Ionic Bonds Covalent Bonds

5. Chemical Bonds Section 4.1 Copyright © Cengage Learning. All rights reserved 5 Ionic Bond Chemical bond formed through the transfer of one or more electrons from one atom or group of atoms to another atom or group of atoms. Ionic Compound –A compound in which ionic bonds are present.

6. Chemical Bonds Section 4.1 Copyright © Cengage Learning. All rights reserved 6 Covalent Bond Chemical bond formed through the sharing of one or more pairs of electrons between two atoms. Molecular Compound (Covalent Compound) –A compound in which atoms are joined through covalent bonds.

7. Chemical Bonds Section 4.1 Copyright © Cengage Learning. All rights reserved 7 Bonding Most bonds are not 100% ionic or 100% covalent. Most bonds have some degree of both ionic and covalent character.

8. Chemical Bonds Section 4.1 Copyright © Cengage Learning. All rights reserved 8 Two Fundamental Concepts 1.Not all electrons in an atom participate in bonding. Those that participate are called valence electrons. 2.Certain arrangements of electrons are more stable than others, as is explained by the octet rule.

9. Section 4.2 Valence Electrons and Lewis Symbols Copyright © Cengage Learning. All rights reserved 9 Valence Electron An electron in the outermost electron shell of a representative element or noble-gas element. In these representative elements or nobel gases the valence electrons are found in either s or p subshells.

10. Section 4.2 Valence Electrons and Lewis Symbols Copyright © Cengage Learning. All rights reserved 10 Lewis Symbol Chemical symbol of an element surrounded by dots equal in number to the number of valence electrons present in atoms of the element.

11. Section 4.2 Valence Electrons and Lewis Symbols Copyright © Cengage Learning. All rights reserved 11 Lewis Symbols for Selected Representative and Noble-Gas Elements

12. Section 4.2 Valence Electrons and Lewis Symbols Copyright © Cengage Learning. All rights reserved 12 Concept Check Determine the number of valence electrons in each of the following elements: Ca Se C

13. Section 4.2 Valence Electrons and Lewis Symbols Copyright © Cengage Learning. All rights reserved 13 Concept Check Determine the number of valence electrons in each of the following elements: Ca 2 valence electrons (4s 2 ) Se 6 valence electrons (4s 2 4p 4 ) C 4 valence electrons (2s 2 2p 2 )

14. Section 4.2 Valence Electrons and Lewis Symbols Copyright © Cengage Learning. All rights reserved 14 Three Important Generalizations About Valence Electrons 1.Representative elements in the same group have the same number of valence electrons. 2.The number of valence electrons for representative elements is the same as the Roman numeral periodic-table group number. 3.The maximum number of valence electrons for any element is eight.

15. Section 4.2 Valence Electrons and Lewis Symbols Copyright © Cengage Learning. All rights reserved 15 Concept Check Write Lewis symbols for the following elements: O P F

16. Section 4.2 Valence Electrons and Lewis Symbols Copyright © Cengage Learning. All rights reserved 16 Concept Check Write Lewis symbols for the following elements: O P F

17. Section 4.3 The Octet Rule Copyright © Cengage Learning. All rights reserved 17 Certain arrangements of valence electrons are more stable than others. The valence electron configurations of the noble gases are considered the most stable of all valence electron configurations.

18. Section 4.3 The Octet Rule Copyright © Cengage Learning. All rights reserved 18 Octet Rule In forming compounds, atoms of elements lose, gain, or share electrons in such a way as to produce a noble-gas electron configuration for each of the atoms involved.

19. Section 4.4 The Ionic Bond Model Copyright © Cengage Learning. All rights reserved 19 Ion An atom (or group of atoms) that is electrically charged as a result of the loss or gain of electrons. If an atom gains one or more electrons, it becomes a negatively charged ion. If an atom loses one or more electrons, it becomes a positively charged ion.

20. Section 4.4 The Ionic Bond Model Copyright © Cengage Learning. All rights reserved 20

21. Section 4.4 The Ionic Bond Model Copyright © Cengage Learning. All rights reserved 21 Concept Check Give the chemical symbol for each of the following ions. a)The ion formed when a potassium atom loses one electron. b)The ion formed when a sulfur atom gains two electrons.

22. Section 4.4 The Ionic Bond Model Copyright © Cengage Learning. All rights reserved 22 Concept Check Give the chemical symbol for each of the following ions. a)The ion formed when a potassium atom loses one electron. K + b)The ion formed when a sulfur atom gains two electrons. S 2–

23. Section 4.5 The Sign and Magnitude of Ionic Charge Copyright © Cengage Learning. All rights reserved 23 Atoms tend to gain or lose electrons until they have obtained an electron configuration that is the same as that of a noble gas.  Example: K + ( 1s 2 2s 2 2p 6 3s 2 3p 6 )  Lost one electron to obtain electron configuration for Ar ( 1s 2 2s 2 2p 6 3s 2 3p 6 ).

24. Section 4.5 The Sign and Magnitude of Ionic Charge Copyright © Cengage Learning. All rights reserved 24 1.Metal atoms containing one, two, or three valence electrons tend to lose electrons to acquire a noble-gas electron configuration. GroupCharge IA1+ IIA 2+ IIIA3+

25. Section 4.5 The Sign and Magnitude of Ionic Charge Copyright © Cengage Learning. All rights reserved 25 2.Nonmetal atoms containing five, six, or seven valence electrons tend to gain electrons to acquire a noble-gas electron configuration. GroupCharge VIIA1– VIA 2– VA3–

26. Section 4.5 The Sign and Magnitude of Ionic Charge Copyright © Cengage Learning. All rights reserved 26 3.Elements in Group IVA occupy unique positions relative to the noble gases (could gain or lose four electrons).

27. Section 4.5 The Sign and Magnitude of Ionic Charge Copyright © Cengage Learning. All rights reserved 27 Isoelectronic Species A series of ions/atoms containing the same number and configuration of electrons. O 2-, F -, Ne, Na +, Mg 2+, and Al 3+ 1s 2 2s 2 2p 6

28. Section 4.5 The Sign and Magnitude of Ionic Charge Copyright © Cengage Learning. All rights reserved 28 Isoelectronic Species Mg 2+ and Ne

29. Section 4.5 The Sign and Magnitude of Ionic Charge Copyright © Cengage Learning. All rights reserved 29 Concept Check Choose an alkali metal, an alkaline earth metal, a noble gas, and a halogen so that they constitute an isoelectronic series when the metals and halogen are written as their most stable ions. What is the electron configuration for each species? Determine the number of electrons for each species. Determine the number of protons for each species.

30. Section 4.6 Lewis Structures for Ionic Compounds Copyright © Cengage Learning. All rights reserved 30 Formation of an Ionic Compound Ion formation requires the presence of two elements: –A metal that can donate electrons. –A nonmetal that can accept electrons. The electrons lost by the metal are the same ones gained by the nonmetal. The positive and negative ions simultaneously formed from such electron transfer attract one another.

31. Section 4.6 Lewis Structures for Ionic Compounds Copyright © Cengage Learning. All rights reserved 31 Lewis Structure Combination of Lewis symbols that represents either the transfer or the sharing of electrons in chemical bonds.

32. Section 4.6 Lewis Structures for Ionic Compounds Copyright © Cengage Learning. All rights reserved 32 The Reaction Between Sodium and Chlorine

33. Section 4.6 Lewis Structures for Ionic Compounds Copyright © Cengage Learning. All rights reserved 33 The Reaction Between Sodium and Oxygen

34. Section 4.6 Lewis Structures for Ionic Compounds Copyright © Cengage Learning. All rights reserved 34 The Reaction Between Calcium and Chlorine

35. Section 4.7 Chemical Formulas for Ionic Compounds Copyright © Cengage Learning. All rights reserved 35 Ionic compounds are always neutral; no net charge is present. The ratio in which positive and negative ions combine is the ratio that achieves charge neutrality for the resulting compound.

36. Section 4.7 Chemical Formulas for Ionic Compounds Copyright © Cengage Learning. All rights reserved 36 Writing Chemical Formulas for Ionic Compounds 1.The symbol for the positive ions is always written first. 2.The charges on the ions that are present are not shown in the formula. 3.The subscripts in the formula give the combining ratio for the ions.

37. Section 4.7 Chemical Formulas for Ionic Compounds Copyright © Cengage Learning. All rights reserved 37 Example Compound formed between Li + and O 2– –Need two Li + to balance out the 2- charge on oxygen. Formula is Li 2 O.

38. Section 4.7 Chemical Formulas for Ionic Compounds Copyright © Cengage Learning. All rights reserved 38 Concept Check Determine the chemical formula for the compound that is formed when each of the following pairs of ions interact. Ba 2+ and Cl – Fe 3+ and O 2– Pb 4+ and O 2–

39. Section 4.7 Chemical Formulas for Ionic Compounds Copyright © Cengage Learning. All rights reserved 39 Concept Check Determine the chemical formula for the compound that is formed when each of the following pairs of ions interact. Ba 2+ and Cl – BaCl 2 Fe 3+ and O 2– Fe 2 O 3 Pb 4+ and O 2– PbO 2

40. Section 4.8 The Structure of Ionic Compounds Copyright © Cengage Learning. All rights reserved 40 Solid Ionic Compounds Consists of positive and negative ions arranged in such a way that each ion is surrounded by nearest neighbors of the opposite charge. Any given ion is bonded by electrostatic attractions to all the other ions of opposite charge immediately surrounding it.

41. Section 4.8 The Structure of Ionic Compounds Copyright © Cengage Learning. All rights reserved 41 Sodium Chloride (NaCl)

42. Section 4.8 The Structure of Ionic Compounds Copyright © Cengage Learning. All rights reserved 42 Formula Unit Smallest whole-number repeating ratio of ions present in an ionic compound that results in charge neutrality. Chemical formulas for ionic compounds represent the simplest ratio of ions present.

43. Section 4.8 The Structure of Ionic Compounds Copyright © Cengage Learning. All rights reserved 43 Cross-Section of NaCl

44. Section 4.9 Recognizing and Naming Binary Ionic Compounds Copyright © Cengage Learning. All rights reserved 44 Binary Compounds:  Composed of two elements  Ionic and covalent compounds included Binary Ionic Compounds:  Metal-nonmetal  Metal is always present as the positive ion, and the nonmetal is always present as the negative ion. Naming Compounds

45. Section 4.9 Recognizing and Naming Binary Ionic Compounds Copyright © Cengage Learning. All rights reserved 45 The full name of the metallic element is given first, followed by a separate word containing the stem of the nonmetallic element name and the suffix –ide. Naming Ionic Compounds

46. Section 4.9 Recognizing and Naming Binary Ionic Compounds Copyright © Cengage Learning. All rights reserved 46 Names of Selected Common Nonmetallic Ions

47. Section 4.9 Recognizing and Naming Binary Ionic Compounds Copyright © Cengage Learning. All rights reserved 47 KClPotassium chloride MgBr 2 Magnesium bromide CaOCalcium oxide Examples

48. Section 4.9 Recognizing and Naming Binary Ionic Compounds Copyright © Cengage Learning. All rights reserved 48 Metals in these compounds form more than one type of positive charge. Charge on the metal ion must be specified. Roman numeral indicates the charge of the metal cation (positively charged ion). Transition metal cations usually require a Roman numeral. Naming Ionic Compounds (for Metals with Variable Charges)

49. Section 4.9 Recognizing and Naming Binary Ionic Compounds Copyright © Cengage Learning. All rights reserved 49 CuBrCopper(I) bromide FeSIron(II) sulfide PbO 2 Lead(IV) oxide Examples

50. Section 4.9 Recognizing and Naming Binary Ionic Compounds Copyright © Cengage Learning. All rights reserved 50 Metallic Elements with a Fixed Ionic Charge

51. Section 4.9 Recognizing and Naming Binary Ionic Compounds Copyright © Cengage Learning. All rights reserved 51 Exercise Name each of the following compounds: K 2 S Fe 2 O 3 CoCl 2

52. Section 4.9 Recognizing and Naming Binary Ionic Compounds Copyright © Cengage Learning. All rights reserved 52 Exercise Name each of the following compounds: K 2 S potassium sulfide Fe 2 O 3 iron(III) oxide CoCl 2 cobalt(II) chloride

53. Section 4.10 Polyatomic Ions Copyright © Cengage Learning. All rights reserved 53 Ion formed from a group of atoms (held together by covalent bonds) through loss or gain of electrons. Polyatomic Ion

54. Section 4.10 Polyatomic Ions Copyright © Cengage Learning. All rights reserved 54 Must be memorized (see Table 4.3 on pg. 99 in text). Examples of compounds containing polyatomic ions: NaOHSodium hydroxide Mg(NO 3 ) 2 Magnesium nitrate (NH 4 ) 2 SO 4 Ammonium sulfate Polyatomic Ions

55. Section 4.10 Polyatomic Ions Copyright © Cengage Learning. All rights reserved 55 1.Most of the polyatomic ions have a negative charge. 2.Two of the negatively charged polyatomic ions, OH – and CN –, have names ending in –ide and the rest of them have names ending in either – ate or –ite. Generalizations

56. Section 4.10 Polyatomic Ions Copyright © Cengage Learning. All rights reserved 56 3.A number of –ate, –ite pairs of ions exist. The – ate ion always has one more oxygen atom than the –ite ion. Both the –ate and –ite ions of a pair carry the same charge. 4.A number of pairs of ions exist wherein one member of the pair differs from the other by having a hydrogen atom present. In such pairs, the charge on the ion that contains hydrogen is always 1 less than that on the other ion. Generalizations

57. Section 4.11 Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions Copyright © Cengage Learning. All rights reserved 57 Determined in the same way as those for ionic compounds that contain monatomic ions. The positive and negative charges present must add to zero.  Na + and OH – form NaOH.  Mg 2+ and NO 3 – form Mg(NO 3 ) 2.  NH 4 + and SO 4 2– form (NH 4 ) 2 SO 4.

58. Section 4.11 Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions Copyright © Cengage Learning. All rights reserved 58 Exercise Which of the following compounds is named incorrectly? a) KNO 3 potassium nitrate b) TiO 2 titanium(II) oxide c) Sn(OH) 4 tin(IV) hydroxide d) (NH 4 ) 2 SO 3 ammonium sulfite e) CaCrO 4 calcium chromate

59. Section 4.11 Chemical Formulas and Names for Ionic Compounds Containing Polyatomic Ions Copyright © Cengage Learning. All rights reserved 59 Exercise Which of the following compounds is named incorrectly? a) KNO 3 potassium nitrate b) TiO 2 titanium(II) oxide c) Sn(OH) 4 tin(IV) hydroxide d) (NH 4 ) 2 SO 3 ammonium sulfite e) CaCrO 4 calcium chromate titanium(IV) oxide